A1-L portion of buffer is made up of an acid whose pka = 5.1 with (HA) =1M and (A-] = 1 M. Which solution will make the buffer exceed its capacity? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. 0.25 L of 1 M HCI a 0.25 L of 1 M NaOH 1L of 0.1 M HCI d. 1l of 0.1 M NaOH 1L of 1.1 M HCI

A1-L portion of buffer is made up of an acid whose pka = 5.1 with (HA) =1M and (A-] = 1 M. Which solution will make the buffer exceed its capacity? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. 0.25 L of 1 M HCI a 0.25 L of 1 M NaOH 1L of 0.1 M HCI d. 1l of 0.1 M NaOH 1L of 1.1 M HCI

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Part A Which set of compounds would form a buffer in aqueous solution? Drag each item to the appropriate bin. Buffer HCN and KCN NaBr and KBr KF and KOH HCOOH and HCOOK NaF and KF Not a buffer HBr and NaBr HF and KCI Reset Help
What is the hydroxide ion concentration in a solution that containing 0.50 mole of ammonium hydroxide and 0.05 mole of ammonium chloride per liter of solution? Since the pKb of ammonium hydroxide is 4.75? and What is the type of buffer solution? a- 1. 54 x 10-4 M. basic buffer b- 1.77 x 10-4 M. acidic buffer c- 1.77 x 10-4 M. basic buffer d- 1. 54x 10-4 M. acidic buffer الاختيارات b a O C d O
For the weak acid equilibrium HA(aq) H*(aq) + A^(aq) A buffer is made containing HA and A". If the [HA] increases and the [A] decreases, a. the pka will increase b. both the pH and pka will increase C. the pH will increase d. the pH will decrease e. the pka will decrease
25). One of your classmates, Chem 109 student said, “I can make a perchlorate buffer using equal amount of 0.1 M HCIO4 and 0.1 M NaCIO4." Will the solution prepared properly by this student functions as a buffer? Another word, can this solution be a buffer? а. yes d. need only ClIO, to make the buffer. c. need only HCIO, to make a perchlorate buffer. e. none of the above b. no
Which of the following is NOT a buffer solution? Select one: O A. 5.0 mL 1.0 M HBr + 15.00 mL 1.0 M CH3C00-Na+ O B. 10.0 mL 1.0M CH3COOH + 10.0 mL 1.0 M NAOH Oc. 15.0 mL 1.0 M CH3COOH + 5.00 mL 1.0 M CH3C00-Na+ O D. All of the choices are buffer solutions. O E 10.0 mL 1.0M CH3COOH + 10.0 mL 1.0 M CH;CO0-Na+
Pp
determine the volume of 0.2 M sodium acetate required to be added to prepapre 100 mL of 0.2 M acetate buffer at ph 4.2? Use the table as a reference.
22. Which of the following mixture could be considered as a buffer? Hint: Try to react each mixture (if possible) and look for a pair that could be components for the buffer c. HC1 + CF d. CH3COO+ OH- a. NH4C1 + NAOH b. NH3 + NaOH 23. What is the pH of a buffer solution containing 0.25 M acetic acid and 0.030 M sodium acetate? The acid dissociation constant for acetic acid is equal to 1.8 x 10 Hint no dilution occurred a. 3.82 b. 5.67 C. 10.18 d. 8.34
What is the effective pH range for a sodium acetate/acetic acid buffer? Ka = 1.80 x 105. %3D Enter your answer to three decimals. to
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8. Which of the four systems formed a buffer (at least initially)? Explain why
While buffer preparation, the buffer solution is 0.1M with a pH of 6.70. What is the correct system to prepare the target buffer? Afterwards, what are the concentrations of the acidic and basic species in the buffer (in M)? a. H3PO4 and H₂PO4- b. H₂PO4 and HPO4²- c. HPO4²- and PO4³-